Versatile Poly(Diallyl Dimethyl Ammonium Chloride)-Layered Nanocomposites for Removal of Cesium in Water Purification

In this work, we elucidate polymer-layered hollow Prussian blue-coated magnetic nanocomposites as an adsorbent to remove radioactive cesium from environmentally contaminated water. To do this, Fe3O4 nanoparticles prepared using a coprecipitation method were thickly covered with a layer of cationic polymer to attach hollow Prussian blue through a self-assembly process. The as-synthesized adsorbent was confirmed through various analytical techniques. The adsorbent showed a high surface area (166.16 m2/g) with an excellent cesium adsorbent capacity and removal efficiency of 32.8 mg/g and 99.69%, respectively. Moreover, the superparamagnetism allows effective recovery of the adsorbent using an external magnetic field after the adsorption process. Therefore, the magnetic adsorbent with a high adsorption efficiency and convenient recovery is expected to be effectively used for rapid remediation of radioactive contamination.


Introduction
Multifunctional polymer nanocomposites cover a very wide range of polymer matrices and hybrid polymer materials for their industrial applications [1,2].
The release of radionuclides, including fission products, from the long-term use of nuclear fuels and occasional nuclear disasters, such as at Chernobyl and the Fukushima Daiichi nuclear power plants, is an emerging issue [1][2][3][4].In particular, radioactive cesium ( 137 Cs), a fission product formed in nuclear reactors, is a problematic contaminant due to its high radioactivity, relatively long half-life (30.2 years), and bioavailability [5][6][7]. 137Cs can cause a number of significant health problems, including carcinoma of the kidney, liver, renal functions, and bladder as well as cardiovascular disease and gastrointestinal distress [8][9][10][11].
Various materials have been investigated for the removal of 137 Cs, including polymers, zeolites, clay minerals, silica, and other nanomaterials [12][13][14].However, these are unsuitable for column loading and are not easy to separate from aqueous solutions by filtration or centrifugation after cesium adsorption [4].
Prussian blue (PB) is a low-cost adsorbent with a strong affinity and high selectivity for cesium.It is also a U.S. Food and Drug Administration (FDA) approved drug employed for the handling of radioactive exposure [15] and has the potential for effective remediation of cesium.There are many reports on PB-based composites for the removal of radioactive cesium, such as PB/graphene foam [16], PB/silica [7,17], PB/glass pores [18], and PB/Alginate bead [19].However, all of these adsorbents are either hard to synthesize or too expensive for large-scale applications.Magnetic separation, which has been used for the removal of cesium, is a fast, easy, and efficient method to recover an adsorbent.Combining PB and magnetic particles for the removal of radioactive cesium has many advantages.PB can selectively remove 137 Cs and the adsorbent can be easily separated from environmentally contaminated water using an external magnet.
In the present study, a novel nanocomposite material composed of PB/poly(diallyl dimethyl ammonium chloride) (PDDA)-coated magnetic particles (Fe 3 O 4 ) was synthesized for efficient adsorption of 137 Cs from an aqueous solution.The synthesized adsorbent was characterized using different techniques (e.g., XRD, FTIR, and TEM) and the effect of adsorbent dosage and pH on the removal efficiency of 137 Cs was investigated.The developed adsorbent was recovered easily using an external magnet and showed a high adsorption capacity that can help solve the difficulty of recovering existing adsorbent materials.

Characterization
A transmission electron microscopy (TEM) analysis was performed using a Tecnai G2 (FEI, Eindhoven, The Netherland) microscope at an accelerating voltage of 200 kV and equipped with an energy dispersive spectrometer (EDS, Oxford Instruments, Oxford, UK).Fourier-transform infrared spectroscopy (FTIR) was analyzed using a Jasco-6600 spectrometer (JASCO, Weinheim, Germany).
The hydrodynamic diameter and zeta potential measurements were carried out using a dynamic light scattering measurement collected on a Zetasizer Nano ZS (Malvern, UK).The X-ray diffraction (XRD) patterns were mainly collected using a Bruker D2 PHASER (Hamburg, Germany) diffractometer with Cu K(alpha) radiation.The Brunauer-Emmett-Teller (BET) surface area and average pore diameter were obtained from the N 2 adsorption/desorption isotherm using a fully automatic physisorption analyzer (ASAP 2020, Micromeritics Instrument Corp., Norcross, GA, USA).

Preparation of Magnetic PDDA@Fe 3 O 4
PDDA-coated magnetic particles were prepared according to a previous report [20].A solution (20 mL) containing FeCl 2 •4H 2 O (0.8 g), FeCl 3 •6H 2 O (2.16 g), and PDDA (1.0%, v/v) was deoxygenated by bubbling with nitrogen gas for 10 min, followed by heating to 80 • C. Subsequently, 10 mL of 2% NH 4 OH was added quickly to the heated solution, which was left to stir for another 1 h.After cooling to room temperature, the obtained PDDA-coated Fe 3 O 4 nanoparticles (NPs) were isolated using a magnet field and washed three times with deionized water.Finally, the nanoparticles were dried at comfortable room temperature.

Synthesis of Mesocrystal and Hollow PB Particles
For the synthesis of mesocrystal Prussian blue (MPB) [21], 3 g of PVP and 131.7 mg of K 3 [Fe(CN) 6 ]•3H 2 O were added into a 0.1 M HCl solution (40 mL) under magnetic stirring, and a clear solution was obtained after 1 h.The solution was then heated in an oven at 80 • C for 20 h.The precipitate formed was then collected through centrifugation, washed with distilled water and ethanol two times, and dried at room temperature for 12 h.Hollow Prussian blue (HPB) particles were synthesized by controlled chemical etching of MPB particles [21].In brief, 20 mg of MPB and 100 mg PVP were added to a 1.0 M HCl solution (20 mL) under magnetic stirring.After 1 h, the solution was transferred into a stainless autoclave and heated at 135 • C for 2.5 h.The HPB particles that were precipitated from the solution were subsequently collected by centrifugation, washed with distilled water and ethanol two times, and then dried at comfortable room temperature for 12 h.

Synthesis of PB@PDDA@Fe 3 O 4 Composite
To synthesize the composite nanoparticles, 1 g of PDDA@Fe 3 O 4 was mainly dispersed in 10 mL of distilled water, and 0.01 M HCl was added to adjust the pH to 6.Then, 3 g of MPB or HPB particles were added to the above solution and 0.01 M NaOH was added to adjust the pH to 6.The slurry obtained was thoroughly mixed at room temperature in a 50 mL polypropylene tube.The MPB or HPB particles were attached to the surface of PDDA@Fe 3 O 4 due to the electrostatic interaction.The obtained HPB@PDDA@Fe 3 O 4 composite was separated from the solution using an external magnet (1.4 teslas) and washed several times with distilled water.

Adsorption Experiments
The adsorption isotherms were investigated using batch experiments with a non-radioactive isotope, 133 Cs.The initial Cs concentration varied from 1-200 ppm.Adsorbent (10 mg) was added to the Cs solution (4 mL).After equilibrating for 12 h, the adsorbent was separated by a magnet and the residual Cs concentration in the solution was analyzed by inductively coupled plasma mass spectrometry (ICP-MS, PerkinElmer ELAN6100, SCIEX PerkinElmer, Beaconsfield, UK).A radioactive 137 Cs adsorption experiment is given in detail in the supporting information.All experiments were conducted 3 to 5 times.

Radioactive 137 Cs Decontamination
Different amounts of HPB@PDDA@Fe 3 O 4 composite (0.5, 2, or 5 mg) were added to 10 mL of the 137 Cs aqueous solution (100 Bq/g); the concentrations of PB NPs/mL of the 137 Cs solution were 0.05, 0.2, 0.5 mg/mL, respectively.After adsorption of 137 Cs for 12 h, the adsorbent was removed using an external magnet.The solution concentrations of the 137 Cs before and after treatment with the adsorbents were analyzed using a high-purity germanium (HPGe) detector (Canberra Inc., Meriden, CT, USA).In particular, we measured more than 3000 counts per second (cps) in each experiment for 1 h.

The Influence of pH on the Removal of 137 Cs
The removal of 137 Cs as a function of solution pH ranging from 4-10 was prepared by adjusting the pH using HCl and NH 4 OH.The initial 137 Cs concentration was 100 Bq/g.All experiments were equilibrated for 12 h with stirring.The nanocomposite was then separated from the solution using a magnet, and the residual 137 Cs concentration was measured using a HPGe detector (Canberra Inc., Meriden, CT, USA).

Fabrication of the Magnetic Adsorbent
Figure 1 shows a schematic representation of the synthesis of PB@PDDA@Fe 3 O 4 .The PDDA@ Fe 3 O 4 composite was prepared via a precipitation reaction.The negatively charged PB (MPB or HPB) was added in excess to a smaller amount of positively charged PDDA@ Fe 3 O 4 , and the surface area of the positively charged PDDA@Fe 3 O 4 was completely covered by negatively charged PB via self-assembly.

Fabrication of the Magnetic Adsorbent
Figure 1 shows a schematic representation of the synthesis of PB@PDDA@Fe3O4.The PDDA@ Fe3O4 composite was prepared via a precipitation reaction.The negatively charged PB (MPB or HPB) was added in excess to a smaller amount of positively charged PDDA@ Fe3O4, and the surface area of the positively charged PDDA@Fe3O4 was completely covered by negatively charged PB via selfassembly.The TEM image of the PDDA@Fe3O4 composite showed aggregated particles with a mean diameter of 200-300 nm, and the subunits were smaller spherical nanocrystals with a size of about 10 nm (Figure 2a,b).HRTEM images (Figure 2b) of the subunits and their corresponding fast Fourier transform (FFT) patterns (Figure 2b inset) indicated the presence of Fe3O4; the spacing of the lattice planes were calculated to be 0.25 nm, which corresponds to the families of crystal planes of Fe3O4.The FFT pattern and spacing of the lattice planes showed exactly the same diffraction patterns compared to Fe3O4 (Figure S1).
Two forms of PB NPs were used: MPB and HPB.MPB was achieved by direct dissociation of a single-source precursor K3[Fe(CN)6] with PVP as a capping and reducing agent.The whole reaction was based on the partial decomposition and reduction of K3[Fe(CN)6] in acidic solution with the addition of PVP.[Fe(CN)6] 3− ions were slowly dissociated into Fe 3+ ions in acidic solution and the Fe 3+ ions were subsequently reduced into Fe 2+ ions by the weak reducer (PVP).Finally, Prussian blue was synthesized through the recrystallization of small particles by the assistance of PVP.MPB was chemically etched with HCl to create HPB with interior hollow cavities.The surface of the HPB (Figure S2c,d) was much rougher than MPB (Figure S2a,b) and the particles size was smaller because of chemical etching.When H + ions diffused into the MPB, the local concentration of H + ions in the center part of the MPB was higher than that of the particle surface.The etching rate of Prussian blue in the center became relatively high, thereby reshaping the interior hollow pore.The TEM image of the HPB (Figure 2c) displayed a network of connected particles.The corresponding selected area electron diffraction (SAED) pattern (Figure 2c inset) showed a diffused ring pattern, indicating a polycrystalline nature [22].Figure 2d,e shows that the HPB particles were successfully decorated onto the surface of the PDDA@Fe3O4 composite.The coating of PDDA onto the Fe3O4 particles provided a positively charged surface, which could combine easily with the HPB nanoparticles because of their electronegative nature (Figure 2e).The EDS spectra (Figure 2f) of a bright field TEM image revealed that the nanocomposite consisted of Fe and O in Fe3O4 area and Fe, C, and N in the HPB area (as indicated in Figure 2e).The TEM image of the PDDA@Fe 3 O 4 composite showed aggregated particles with a mean diameter of 200-300 nm, and the subunits were smaller spherical nanocrystals with a size of about 10 nm (Figure 2a,b).HRTEM images (Figure 2b) of the subunits and their corresponding fast Fourier transform (FFT) patterns (Figure 2b inset) indicated the presence of Fe 3 O 4 ; the spacing of the lattice planes were calculated to be 0.25 nm, which corresponds to the families of crystal planes of Fe 3 O 4 .The FFT pattern and spacing of the lattice planes showed exactly the same diffraction patterns compared to Fe 3 O 4 (Figure S1).
Two forms of PB NPs were used: MPB and HPB.MPB was achieved by direct dissociation of a single-source precursor K 3 [Fe(CN) 6 ] with PVP as a capping and reducing agent.The whole reaction was based on the partial decomposition and reduction of K 3 [Fe(CN) 6 ] in acidic solution with the addition of PVP.[Fe(CN) 6 ] 3− ions were slowly dissociated into Fe 3+ ions in acidic solution and the Fe 3+ ions were subsequently reduced into Fe 2+ ions by the weak reducer (PVP).Finally, Prussian blue was synthesized through the recrystallization of small particles by the assistance of PVP.MPB was chemically etched with HCl to create HPB with interior hollow cavities.The surface of the HPB (Figure S2c,d) was much rougher than MPB (Figure S2a,b) and the particles size was smaller because of chemical etching.When H + ions diffused into the MPB, the local concentration of H + ions in the center part of the MPB was higher than that of the particle surface.The etching rate of Prussian blue in the center became relatively high, thereby reshaping the interior hollow pore.The TEM image of the HPB (Figure 2c) displayed a network of connected particles.The corresponding selected area electron diffraction (SAED) pattern (Figure 2c inset) showed a diffused ring pattern, indicating a polycrystalline nature [22].Figure 2d,e shows that the HPB particles were successfully decorated onto the surface of the PDDA@Fe 3 O 4 composite.The coating of PDDA onto the Fe 3 O 4 particles provided a positively charged surface, which could combine easily with the HPB nanoparticles because of their electronegative nature (Figure 2e).The EDS spectra (Figure 2f) of a bright field TEM image revealed that the nanocomposite consisted of Fe and O in Fe 3 O 4 area and Fe, C, and N in the HPB area (as indicated in Figure 2e).

Morphological and Surface Studies
The surface coating also affected the zeta potential and particle size.The zeta potential values of the Fe3O4, PDDA@Fe3O4, MPB@PDDA@Fe3O4, and HPB@PDDA@Fe3O4 in water were −40, 33, −29 and −38 mV, respectively (Figure 3a). Figure 2b exhibits a photographic image of an aqueous solution of Fe3O4, PDDA@Fe3O4, MPB@PDDA@Fe3O4, and HPB@PDDA@Fe3O4.After the reaction between Fe3O4 and PB, the aqueous solution turned a blue or dark green, indicating PB on the surface of the magnetic nanoparticles (MNPs).
The FTIR spectra also demonstrated the successful coating of MPB or HPB on the PDDA@Fe3O4 surface (Figure 3c).The absorption bands at 3375-3787 and 1615 cm −1 refer to the O-H stretching mode and H-O-H bending mode due to water molecules.The prominent peak intensity of PB at 2076 cm −1 was observed in HPB@PDDA@Fe3O4 (Figure 3c).The common characteristics of PB were observed from the absorption band at 2076 cm −1 owing to the stretching vibration of the C≡N group [22].For the PDDA sample, a strong band at ~3440 cm −1 was attributed mainly to -NR3 + stretching vibration, and the bands around the 3000-2800 cm −1 region were assigned to the C-H bending, as shown in Figure 3c [23].The presence of Fe-O bond from Fe3O4 was also able to be seen at 539 cm −1 for all those samples with Fe3O4.From the FTIR results, the presence of both Fe3O4 and HPB were identified for all samples.

Morphological and Surface Studies
The surface coating also affected the zeta potential and particle size.The zeta potential values of the Fe 3 O 4 , PDDA@Fe 3 O 4 , MPB@PDDA@Fe 3 O 4 , and HPB@PDDA@Fe 3 O 4 in water were −40, 33, −29 and −38 mV, respectively (Figure 3a). Figure 2b exhibits a photographic image of an aqueous solution of Fe 3 O 4 , PDDA@Fe 3 O 4 , MPB@PDDA@Fe 3 O 4, and HPB@PDDA@Fe 3 O 4 .After the reaction between Fe 3 O 4 and PB, the aqueous solution turned a blue or dark green, indicating PB on the surface of the magnetic nanoparticles (MNPs).
The FTIR spectra also demonstrated the successful coating of MPB or HPB on the PDDA@Fe3O4 surface (Figure 3c).The absorption bands at 3375-3787 and 1615 cm −1 refer to the O-H stretching mode and H-O-H bending mode due to water molecules.The prominent peak intensity of PB at 2076 cm −1 was observed in HPB@PDDA@Fe3O4 (Figure 3c).The common characteristics of PB were observed from the absorption band at 2076 cm −1 owing to the stretching vibration of the C≡N group [22].For the PDDA sample, a strong band at ~3440 cm −1 was attributed mainly to -NR 3 + stretching vibration, and the bands around the 3000-2800 cm −1 region were assigned to the C-H bending, as shown in Figure 3c [23].The presence of Fe-O bond from Fe 3 O 4 was also able to be seen at 539 cm −1 for all those samples with Fe 3 O 4 .From the FTIR results, the presence of both Fe 3 O 4 and HPB were identified for all samples.

Performance Evaluation of Cesium Removal
The uptake of cesium by MPB@PDDA@Fe 3 O 4 and HPB@PDDA@Fe 3 O 4 composites was investigated in the batch experiments.After 12 h of contact, the magnetic composites were easily collected to one side of the vial by positioning a magnet against the vial (Figure 5a).The NPs were rapidly separated within 30 s.This demonstrated that the adsorbent could be very easily recovered using an external magnet.The adsorption capacity of magnetic cesium adsorbents was investigated using Langmuir and Freundlich adsorption isotherm models.The Langmuir model [24] is based on the assumption that all active sites are independent and equivalent, and it indicates a monolayer adsorption process for cesium onto the uniformly adsorbent surface.The nonlinear forms of the equation are written as: where q e and q max are the equilibrium adsorption capacity and monolayer maximum adsorption capacity (mg/g), respectively, and K L is a constant related to the affinity between the adsorbent and the adsorbate.C e is equilibrium concentrations of inactive cesium in the solution.By comparison, the Freundlich adsorption isotherm model [25] is significantly considered to be an empirical equation that describes multilayer adsorption with several types of adsorption sites on the surface of an adsorbent.The model consists of the following equation: where K F and n are the Freundlich constants relative to the multilayer adsorption capacity.The experimental data of HPB@PDDA@Fe 3 O 4 and MPB@PDDA@Fe 3 O 4 composites were a better fit to the Langmuir model (R 2 = 0.91 and 0.90, respectively) than the Freundlich model (R 2 = 0.79 and 0.86, respectively).The MPB@PDDA@Fe 3 O 4 and HPB@PDDA@Fe 3 O 4 possessed a q max of 25.6 and 32.8 mg/g, respectively (Figure 5b).

Performance Evaluation of Cesium Removal
The uptake of cesium by MPB@PDDA@Fe3O4 and HPB@PDDA@Fe3O4 composites was investigated in the batch experiments.After 12 h of contact, the magnetic composites were easily collected to one side of the vial by positioning a magnet against the vial (Figure 5a).The NPs were rapidly separated within 30 s.This demonstrated that the adsorbent could be very easily recovered using an external magnet.The adsorption capacity of magnetic cesium adsorbents was investigated using Langmuir and Freundlich adsorption isotherm models.The Langmuir model [24] is based on the assumption that all active sites are independent and equivalent, and it indicates a monolayer adsorption process for cesium onto the uniformly adsorbent surface.The nonlinear forms of the equation are written as: where qe and qmax are the equilibrium adsorption capacity and monolayer maximum adsorption capacity (mg/g), respectively, and KL is a constant related to the affinity between the adsorbent and the adsorbate.Ce is equilibrium concentrations of inactive cesium in the solution.By comparison, the Freundlich adsorption isotherm model [25] is significantly considered to be an empirical equation that describes multilayer adsorption with several types of adsorption sites on the surface of an adsorbent.The model consists of the following equation: ( where KF and n are the Freundlich constants relative to the multilayer adsorption capacity.The experimental data of HPB@PDDA@Fe3O4 and MPB@PDDA@Fe3O4 composites were a better fit to the Langmuir model (R 2 = 0.91 and 0.90, respectively) than the Freundlich model (R 2 = 0.79 and 0.86, respectively).The MPB@PDDA@Fe3O4 and HPB@PDDA@Fe3O4 possessed a qmax of 25.6 and 32.8 mg/g, respectively (Figure 5b).

Radioactive Cesium Adsorption Studies
Figure 6a shows the efficiency of adsorbents for the removal of 137 Cs from an aqueous solution using different adsorbent concentrations (0.05, 0.2, and 0.5 mg/mL).The initial 137 Cs concentrations were 92.38 Bq/g and 86.44 Bq/g for MPB-and HPB-coated nanoparticles, respectively.For a MPB@PDDA@Fe3O4 composite, the removal of 137 Cs from the solution per gram of adsorbent was increased from 95.17% to 97.77% when increasing the adsorbent concentration from 0.05 to 0.5 mg/mL.In the case of the HPB@PDDA@Fe3O4 composite, the removal efficiency increased from

Radioactive Cesium Adsorption Studies
Figure 6a shows the efficiency of adsorbents for the removal of 137 Cs from an aqueous solution using different adsorbent concentrations (0.05, 0.2, and 0.5 mg/mL).The initial 137 Cs concentrations were 92.38 Bq/g and 86.44 Bq/g for MPB-and HPB-coated nanoparticles, respectively.For a MPB@PDDA@Fe 3 O 4 composite, the removal of 137 Cs from the solution per gram of adsorbent was increased from 95.17% to 97.77% when increasing the adsorbent concentration from 0.05 to 0.5 mg/mL.
In the case of the HPB@PDDA@Fe 3 O 4 composite, the removal efficiency increased from 96.18% to 99.69% with an increase in adsorbent concentration.This higher removal efficiency probably results from the higher surface area of the HPB@PDDA@Fe 3 O 4 compared to the MPB@PDDA@Fe 3 O 4 .The effect of pH on 137 Cs uptake by the HPB@PDDA@Fe 3 O 4 composite was investigated, as shown in Figure 6b.At the three pH values investigated (pH 4, 7, and 10), the HPB@PDDA@Fe 3 O 4 adsorbent removed over 92% of 137 Cs, and a maximum 137 Cs uptake of 98.26% was achieved at pH 7. When the pH further increases or decreases, the adsorption sites become available for cation or anion in ion exchange processes, which leads to difficult cesium adsorption.Even though the removal efficiency of cesium ions is feasible across a wide range of pH values, the best results are achieved at neutrality.
The distribution coefficient (K d ) was defined to analyze the cesium removal ability and adsorption performance of HPB@PDDA@Fe 3 O 4 toward 137 Cs: where C 0 and C f are the initial and final concentrations of Cs in the solution before and after equilibrium contact with the adsorbent, V is the volume of the solution, and M is the mass of the adsorbent used.
For the HPB@PDDA@Fe 3 O 4 composite, the K d was calculated as ~6.4 × 10 5 mL/g, which was an order of magnitude higher than the literature value for the PB adsorbent of 5.2 × 10 4 mL/g [7].Based on these results, we speculate that the resulting hollow adsorbents provide a wider reaction space through which cesium can be adsorbed, thereby increasing the adsorption capacity.96.18% to 99.69% with an increase in adsorbent concentration.This higher removal efficiency probably results from the higher surface area of the HPB@PDDA@Fe3O4 compared to the MPB@PDDA@Fe3O4.The effect of pH on 137 Cs uptake by the HPB@PDDA@Fe3O4 composite was investigated, as shown in Figure 6b.At the three pH values investigated (pH 4, 7, and 10), the HPB@PDDA@Fe3O4 adsorbent removed over 92% of 137 Cs, and a maximum 137 Cs uptake of 98.26% was achieved at pH 7. When the pH further increases or decreases, the adsorption sites become available for cation or anion in ion exchange processes, which leads to difficult cesium adsorption.Even though the removal efficiency of cesium ions is feasible across a wide range of pH values, the best results are achieved at neutrality.The distribution coefficient (Kd) was defined to analyze the cesium removal ability and adsorption performance of HPB@PDDA@Fe3O4 toward 137 Cs: where C0 and Cf are the initial and final concentrations of Cs in the solution before and after equilibrium contact with the adsorbent, V is the volume of the solution, and M is the mass of the adsorbent used.For the HPB@PDDA@Fe3O4 composite, the Kd was calculated as ~6.4 × 10 5 mL/g, which was an order of magnitude higher than the literature value for the PB adsorbent of 5.2 × 10 4 mL/g [7].Based on these results, we speculate that the resulting hollow adsorbents provide a wider reaction space through which cesium can be adsorbed, thereby increasing the adsorption capacity.  13Cs by MPB@PDDA@Fe3O4 and HPB@PDDA@Fe3O4 composites and (b) influence of pH on the uptake of 137 Cs by HPB@PDDA@Fe3O4 composite.

Conclusions
In this study, we successfully synthesized a new adsorbent material that shows a high cesium adsorption efficiency and easy recovery of adsorbents by decorating hollow PB onto a magnetic PDDA@Fe3O4 composite.The hollow PB attached to the outside of the magnetic particles-like a bunch of grapes-can increase the active specific area and consequently improve the cesium adsorption capacity.Furthermore, the excellent magnetic composite property makes it possible to recover the adsorbent effectively and selectively bind cesium from contaminated radioactive wastewater through a magnetic field.In the selective adsorption experiment, the adsorbent, HPB@PDDA@Fe3O4, exhibited an excellent maximum adsorption capacity of 32.8 mg/g and 137 Cs removal efficiency of 99.69%.This new approach for the synthesis of a functional adsorbent can be an important contribution towards the effective removal of 137 Cs.

Conclusions
In this study, we successfully synthesized a new adsorbent material that shows a high cesium adsorption efficiency and easy recovery of adsorbents by decorating hollow PB onto a magnetic PDDA@Fe 3 O 4 composite.The hollow PB attached to the outside of the magnetic particles-like a bunch of grapes-can increase the active specific area and consequently improve the cesium adsorption capacity.Furthermore, the excellent magnetic composite property makes it possible to recover the adsorbent effectively and selectively bind cesium from contaminated radioactive wastewater through a magnetic field.In the selective adsorption experiment, the adsorbent, HPB@PDDA@Fe 3 O 4 , exhibited an excellent maximum adsorption capacity of 32.8 mg/g and 137 Cs removal efficiency of 99.69%.This new approach for the synthesis of a functional adsorbent can be an important contribution towards the effective removal of 137 Cs.

Figure 5 .
Figure 5. (a) Photograph shows the recovery of the composite with an external magnet after Cs adsorption; (b) nonlinear Langmuir (solid lines) and Freundlich (dotted lines) isotherm models.

Figure 5 .
Figure 5. (a) Photograph shows the recovery of the composite with an external magnet after Cs adsorption; (b) nonlinear Langmuir (solid lines) and Freundlich (dotted lines) isotherm models.